A sample of 1.0g of solid `Fe_(2)O_(3) of 80%` purity is dissolved in a moderately concentrated HCl solution which is reduced by zinc dust. The resulting solution required 16.7mL of a 0.1M solution of the oxidant. Calculate the number of electrons taken up by the oxidant.

Options

A. 5
B. 2
C. 4
D. 6

Answer

D

Explanation

`"Weight of pure "Fe_(2)O_(3)=(1xx80)/(100)=0.8g`
`Fe_(2)O_(3)+6HCl rarr 2FeCl_(3)+3H_(2)O`
`2FeCl_(3)+H_(2)overset("Zn dust")rarr 2FeCl_(2)+2HCl`
`Fe^(++)+"Oxidant"rarrFe^(+++)+"reduc tan t"`
`"Eq. wt. of "Fe_(2)O_(3)=("Mol. Wt")/(2)=(160)/(2)=80g`
meq. of `Fe_(2)O_(3)="meq of oxidant"`
,`(0.8)/(80)xx10^(3)=16.7xx0.1(x)`
`therefore x=6`